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(C) For a real gas at high pressure, the van der Waals equation is $P(V - nb) = nRT$.Given: $n = 1 \ mol$, $T = 300 \ K$, $P = 100 \ bar$, $b = 0.005

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$1.02 \quad 2$

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(C) For a real gas at high pressure, the van der Waals equation is $P(V - nb) = nRT$.Given: $n = 1 \ mol$, $T = 300 \ K$, $P = 100 \ bar$, $b = 0.005 \ L \ mol^{-1}$, $R = 0.08314 \ bar \ L \ K^{-1} \ mol^{-1}$.Substituting the values: $100(V - 0.005) = 1 	imes 0.08314 	imes 300$.$100(V - 0.005) = 24.942$.$V - 0.005 = 0.24942$.$V_{real} = 0.25442 \ L$.The ideal volume is $V_{ideal} = \frac{nRT}{P} = \frac{1 	imes 0.08314 	imes 300}{100} = 0.24942 \ L$.Compressibility factor $Z = \frac{PV_{real}}{nRT} = \frac{100 	imes 0.25442}{1 	imes 0.08314 	imes 300} = \frac{25.442}{24.942} \approx 1.02$.$\%$ Deviation of volume $= \frac{V_{real} - V_{ideal}}{V_{real}} 	imes 100 = \frac{0.25442 - 0.24942}{0.25442} 	imes 100 = \frac{0.005}{0.25442} 	imes 100 \approx 1.96 \% \approx 2 \%$.Thus, the values are $Z = 1.02$ and $\%$ deviation $= 2$.

$1 \ mol$ of a real gas is kept at a high pressure of $100 \ bar$ at $300 \ K$. If the van der Waals constant $b$ is $0.005 \ L \ mol^{-1}$, what are the values of the compressibility factor $Z$ of the gas and the $\%$ deviation of volume from ideality?
$Z$ $\%$ Deviation

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$1 \ mol$ of a real gas is kept at a high pressure of $100 \ bar$ at $300 \ K$. If the van der Waals constant $b$ is $0.005 \ L \ mol^{-1}$, what are the values of the compressibility factor $Z$ of the gas and the $\%$ deviation of volume from ideality?$Z$$\%$ Deviation